Deck 1: Matter and Energy an Atomic Perspective

Question 1

A molecule

A)must contain at least two types of atoms.
B)can be an element or a compound.
C)cannot form a solid.
D)cannot be broken into its constituent atoms by any means.
E)can contain only one type of atom.

Answer 1

can be an element or a compound.

Question 2

The law of definite proportions states that

A)compounds such as NO and NO₂ have identical chemical properties.
B)compounds such as NO and NO₂ must have masses that are whole-number multiples of each other.
C)nitrogen and oxygen can combine to form a variety of compounds, such as NO or NO₂.
D)the elements forming a given compound always react in the same proportions.
E)only one compound can be produced when two elements combine.

Answer 2

the elements forming a given compound always react in the same proportions.

Question 3

An element

A)can be separated into its components by physical methods.
B)has different chemical properties depending on its state.
C)cannot be separated into simpler substances by chemical methods.
D)can also be a compound.
E)exists only as atoms, not as molecules.

Answer 3

cannot be separated into simpler substances by chemical methods.

Question 4

Which of the following does NOT illustrate the law of multiple proportions?

A)The N-to-O mass ratio in NO is 0.875, whereas that in N₂O is 1.75.
B)C₂H₂ has a 12:1 C-to-H mass ratio, while C₂H₆ has a 4:1 C-to-H mass ratio.
C)The ratio of O:C by mass in CO₂ is twice that of CO.
D)If a sample of H₂O contains 16 g of oxygen, a sample of H₂O₂ with the same number of molecules would contain 32 g of oxygen.
E)H₂S and H₂O contain the same mass of hydrogen.

Question 5

For a hypothesis to be considered a valid scientific theory, it must

A)summarize experimental data without trying to predict future results.
B)be impossible to prove wrong by experiment.
C)explain widely observed phenomena based on extensive testing.
D)never be modified or expanded.
E)be voted on by the scientific community and accepted by all.

Question 6

Which of the following is NOT an element?

A)Cs
B)Au
C)CS₂
D)Ar
E)Co

Question 7

Table sugar (sucrose, C₁₂H₂₂O₁₁) dissolves in water.This process__________

A)is a chemical change.
B)is a physical change.
C)produces a heterogeneous mixture.
D)is a chemical property of sucrose.
E)converts sucrose to carbon dioxide and water.

Question 8

A pure substance

A)must be composed of atoms of the same type.
B)cannot be separated into simpler substances by physical means.
C)must be a compound.
D)has different chemical properties depending on its source.
E)can have a composition that varies from sample to sample.

Question 9

According to the law of definite proportions,

A)atoms forming a given compound react in variable proportions depending on conditions.
B)different samples of the same compound contain the same proportions of the same elements.
C)all compounds containing the same types of atoms have identical properties.
D)all compounds containing the same types of atoms have relative masses that are whole-number multiples.
E)only one type of molecule can be produced when two elements combine.

Question 10

Which of the following is a homogeneous mixture?

A)an egg
B)smoke
C)beach sand
D)dry ice solid CO₂
E)a salt solution NaCl dissolved in water)

Question 11

Which of the following statements is NOT true?

A)Given that the chemical formula of methanol is CH₄O, the number of carbon atoms in a sample of methanol will be the same as the number of oxygen atoms.
B)If a compound is 75% carbon and 25% hydrogen by mass, 12 g of the compound contains 9 g C and 3 g H.
C)If a compound contains 76 g of chlorine and 12 g of carbon, it will always have a 6.33:1 mass ratio of Cl to C.
D)A compound containing 17.1 g of phosphorus and 58.9 g of chlorine has the same identity as a compound containing 35.7 g P and 204.3 g Cl.
E)A compound containing 106.6 g of copper and 13.4 g of oxygen has the same identity as a compound containing 159.9 g Cu and 20.1 g O.

Question 12

Which of the following illustrates the law of multiple proportions?

A)The mass ratio of O to N in NO₂ is twice that in NO.
B)NO₂ always contains one nitrogen atom and two oxygen atoms.
C)The mass of NO₂ is a small whole-number multiple of the mass of NO.
D)NO and NO₂ have similar chemical and physical properties.
E)NO₂ and N₂O₄ are the same compound.

Question 13

Which of the following is NOT a pure substance?

A)sparkling water
B)gold metal
C)oxygen gas
D)water vapor
E)dry ice solid (CO₂)

Question 14

Which one of the following is a hypothesis?

A)Energy is required to vaporize a liquid.
B)The composition of a pure substance is fixed and definite.
C)Hydrogen gas and oxygen gas can react to form water.
D)A Car's battery must be dead because the car won't start.
E)Matter is composed of atoms.

Question 15

Which of the following is an element?

A)C₆H₁₂O₆
B)HNO₃
C)NaCl
D)CH₄
E)O₃

Question 16

Which of the following is a pure substance?

A)seawater
B)blood
C)brass an alloy of copper and zinc)
D)table sugarsucrose, C₁₂H₂₂O₁₁.
E)beer

Question 17

Which of the following statements is NOT true?

A)The relative numbers of each type of atom in a given compound do not vary.
B)A compound always contains the same mass percentages of its constituent elements.
C)A large sample and a small sample of a given compound contain the same number of each type of atom.
D)A large sample and a small sample of a given compound contain the same types of atoms combined in the same proportions.
E)A large sample and a small sample of a compound share the same chemical formula.

Question 18

Which of the following is a heterogeneous mixture?

A)concrete
B)sweet tea
C)black coffee
D)mercury metal
E)an intravenous (IV) solution

Question 19

Which step is NOT a part of the scientific method?

A)Form a testable hypothesis.
B)Make observations.
C)Conduct reproducible experiments.
D)Identify different factors that affect results.
E)Stop experimentation once the desired results are achieved.

Question 20

A sample of a compound

A)breaks into its constituent atoms during phase changes.
B)is a homogeneous mixture.
C)contains atoms that can be physically separated from each other.
D)contains at least two types of atoms in a constant, fixed ratio.
E)has a variable composition depending on its temperature.

Question 21

Which of the following is a chemical property of copper metal?

A)It conducts heat.
B)It reacts with nitric acid to produce copper(II) nitrate.
C)It melts at 1085 $\degree$ C
D)It conducts electricity.
E)It has an orange color.

Question 22

Which one of the following represents a physical change?

A)Milk turns sour.
B)Rust forms on iron nails.
C)Sugar ferments to form ethanol.
D)An egg begins to smell very bad.
E)Sugar melts and forms a syrupy liquid.

Question 23

Which of the following represents a physical property of water?

A)It boils at 100 $\degree$ C.
B)An electrical current decomposes water into hydrogen gas and oxygen gas.
C)It reacts with iron metal and oxygen to form rust.
D)It reacts with carbon monoxide to form carbon dioxide and hydrogen gas.
E)It is used in photosynthesis.

Question 24

Distillation may be used to separate components in a mixture based on_____

A)solubilities.
B)masses.
C)volatilities.
D)densities.
E)colors.

Question 25

Which of the following is a chemical property of acetone C₃H₆O?

A)It readily evaporates at room temperature.
B)It has a pungent, irritating odor.
C)It can be ignited in oxygen.
D)It boils at 56 $\degree$ C.
E)It is miscible with water.

Question 26

Based on values for the volume per gram of the given materials, which of the following would NOT float in water density = 0.997 g/cm3)?

A)balsa wood
B)cork
C)charcoal
D)human fat
E)ethylene glycol

Question 27

When copper metal is dropped into nitric acid, a blue solution containing copperII) ions is produced along with brown nitrogen monoxide gas.Which of the following is an example of a chemical property?

A)copper's red-orange appearance
B)nitrogen monoxide's irritating odor
C)the blue color of aqueous copper(II) ions
D)the viscosity of nitric acid at room temperature
E)nitric acid's ability to react with copper metal

Question 28

Acetone and water mix to form a homogeneous solution.Acetone has a boiling point of 56 $\degree$ C.Which of the following would be a suitable method for separating acetone from water?

A)filtration
B)combustion
C)distillation
D)scanning tunneling microscopy
E)sublimation

Question 29

Which process would be a practical and effective way to separate beta-carotene, an orange pigment, from hexane liquid?

A)filtration
B)chromatography
C)combustion
D)scanning tunneling microscopy
E)sublimation

Question 30

Extensive properties are

A)dependent on the amount of substance present.
B)identical for all substances.
C)independent of a substance's phase.
D)the physical properties of a substance.
E)dependent on the reactivity of the substance.

Question 31

Which of the following can be separated by filtration?

A)rust particles in water
B)air dispersed in whipped cream
C)alcohol dissolved in water
D)salt dissolved in water
E)nitrogen from air

Question 32

Which represents an extensive property of hydrogen?

A)Hydrogen gas is odorless and colorless.
B)A hydrogen gas molecule is composed of two hydrogen atoms.
C)Hydrogen gas is flammable.
D)Hydrogen releases a given amount of energy when it reacts with oxygen.
E)Hydrogen gas under normal conditions is nonmetallic.

Question 33

Which statement is true regarding ammonia, NH₃?

A)It can also be correctly represented as N₂H₆.
B)It cannot be decomposed into simpler substances by any means.
C)Its decomposition produces three volumes of hydrogen for every one volume of nitrogen.
D)It can be separated into nitrogen and hydrogen atoms using distillation.
E)It is not a stable molecule and does not exist at room temperature.

Question 34

Which of the following is an intensive property of chlorine?

A)It has mass.
B)It boils at - 34 - C.
C)Chlorine gas expands to fill a balloon.
D)The reaction of chlorine with hydrogen releases a given amount of energy.
E)Chlorine gas in a container exerts a given pressure at a given temperature.

Question 35

If you had equal masses of each of the following substances, which would occupy the greatest volume?

A)ice (d = 0.917 g/mL)
B)water (d = 0.997 g/mL)
C)beeswax (d = 0.960 g/mL)
D)cocoa butter (d = 0.910 g/mL)
E)aluminum (d = 2.70 g/mL)

Question 36

Which one of the following represents a chemical change?

A)Mercury(II) oxide is heated up and forms mercury metal and oxygen gas.
B)Rubbing alcohol evaporates.
C)Iodine vapor deposits on a surface.
D)Iron metal is separated from sand using a magnet.
E)Rock salt is pulverized.

Question 37

Which of the following is a chemical property of formaldehyde (CH₂O)?

A)It is flammable.
B)It has a density of 1.09 g/mL.
C)It is colorless.
D)It dissolves in water.
E)It is a gas at room temperature.

Question 38

Which one of the following is NOT an intensive physical property of a pure liquid?

A)boiling point
B)conductivity
C)mass
D)density
E)color

Question 39

Which of the following is a chemical property of platinum?

A)It conducts heat and electricity.
B)It can react with chlorine gas to form platinum(IV) chloride.
C)The difference between its melting and boiling points is 2057 $\degree$ C.
D)It is a gray-white metal.
E)Sound travels through it at a speed of 2680 m/s.

Question 40

Which of the following represents a chemical property of iron?

A)Its density is 7.84 g/cm³.
B)It is magnetic.
C)It reacts with oxygen in moist air.
D)Its melting point is 1538 $\degree$ C.
E)It conducts electricity.

Question 41

Equal amounts of a pure substance undergo the following changes.Which process would you predict releases the greatest amount of energy?

A)deposition (gas $\rightarrow$ solid)
B)vaporization (liquid $\rightarrow$ gas)
C)freezing (liquid $\rightarrow$ solid)
D)condensation (gas $\rightarrow$ liquid)
E)melting (solid $\rightarrow$ liquid)

Question 42

Consider electrons traveling through a copper (Cu) wire at a speed of 0.024 cm/s.What is true about the energy of their motion?

A)It is primarily kinetic.
B)It is primarily potential.
C)It would be unaffected if the speed of the electrons increased.
D)It is strongly affected by gravity.
E)It cannot be used to do work.

Question 43

The chemical formula of dimethyl ether can be represented in different ways.When its formula is written as C₂H₆O,

A)the arrangement of the atoms in the molecule is evident.
B)only the number and type of atoms of each element are given.
C)its structural formula can be deduced.
D)it shows that no other molecules can have that formula.
E)it lists only one of many possible elemental compositions for dimethyl ether.

Question 44

Which of the following statements about energy, work, and heat is NOT true?

A)Adding heat to a sample of matter increases the average kinetic energy of its constituent particles.
B)Thermal energy is the portion of the energy of an object that increases as temperature increases.
C)When an object does work, part of the energy it expends is destroyed as it converts to heat.
D)The energy available from some chemical reactions can be used to do work and/or produce heat.
E)Heat involves the transfer of energy from a hotter object to a cooler one.

Question 45

Work is defined as the exertion of force through a distance.Which of the following is NOT an example of work?

A)Molecules in the air push against the blades of a windmill.
B)Blood is pumped through the circulatory system.
C)Electrons flow against the resistance present in a copper wire.
D)Thermal energy heat) is transferred from a hot stove to the surrounding air.
E)A student lifts a book off of the floor.

Question 46

The space-filling model of a molecule

A)clearly shows bond angles.
B)gives little idea of how atoms are arranged.
C)is best suited for very large molecules.
D)gives an indication of three-dimensional shape.
E)spreads atoms out so they are easy to view.

Question 47

Equal amounts of water undergo the following changes.Which of the following would involve the largest change in energy?

A)Ice is melted to form liquid water at 0 $\degree$ C.
B)Ice at -25 $\degree$ C is heated to 0 $\degree$ C.
C)Water is heated from 25 $\degree$ C to 50 $\degree$ C.
D)Steam at 100 $\degree$ C is cooled and condensed to form liquid water at 85 $\degree$ C.
E)Water at 0 $\degree$ C is heated and vaporized to form steam at 120 $\degree$ C.

Question 48

Equal amounts of water are present under the following conditions.In which case do the water molecules have the highest kinetic energy?

A)as ice at - 10 - C
B)as steam at 100-C
C)in the liquid phase at 80-C
D)in the gas phase at 150-C
E)in the solid phase at 0-C

Question 49

Which statement correctly describes the properties of gaseous helium He)?

A)The gas is not highly compressible even though the atoms do not occupy the entire volume of the container.
B)The gas is highly compressible because there is a lot of empty space between the atoms.
C)The atoms are moving rapidly about the container, giving the gas its definite shape.
D)The gas has a definite volume and shape because the atoms are not moving about the container.
E)A gas takes the shape of the container, but its total volume cannot change.

Question 50

Which of the following is the SI base unit for mass?

A)g
B)kg
C)mg
D)lb
E)m

Question 51

The densities of cork, lead, and water are 0.240 g/cm³, 11.34 g/cm³, and 0.997 g/cm³ at 25 $\degree$ C, respectively.If 20.0 g of lead are placed inside an 85.0 cm³ piece of cork, what is the overall density, and will it float on water?

A)0.466 g/cm³; Yes, it will float.
B)0.235 g/cm³; Yes, it will float.
C)0.211 g/cm³; Yes, it will float.
D)4.25 g/cm³; No, it will not float.
E)2.15 g/cm³; No, it will not float.

Question 52

What type of chemical formula is shown for diethyl ether?

A)molecular
B)structural
C)condensed structural
D)ball-and-stick
E)space-filling

Question 53

Which statement describing the properties of the different phases of a sample of matter is true?

A)The particles in both the gas and liquid phases are highly ordered and in close proximity to one another.
B)The particles in the liquid phase are highly compressible because they can slip past one another.
C)The particles in both the solid and liquid phases are free to assume any shape, and their nearest neighbors change over time.
D)The solid phase is rigid, even though its constituent particles may vibrate a little depending on their temperature.
E)Localized areas of order can form in the gas phase because the particles experience significant attractions to one another.

Question 54

Ethanol and dimethyl ether molecules both contain two carbon atoms, six hydrogen atoms, and one oxygen atom.Which statement is true?

A)Their molecular formulas are different.
B)They show the same physical properties but different chemical properties.
C)The arrangement of the atoms in each type of molecule is different.
D)Their melting points and boiling points are the same.
E)There is no physical method that can distinguish between the two.

Question 55

Which has the highest kinetic energy, assuming all follow the equation KE - ½ mu², where m is the mass and u is the velocity?

A)a one-ton (910 kg) truck traveling at 65 miles per hour (29 m/s)
B)an electron with a mass of 9.11 -10^-27 kg traveling at 2.97 -10⁸ m/s (99% of the speed of light)
C)an oxygen molecule with a mass of 5.31 -10^-26 kg traveling at 394 m/s (roughly its speed at room temperature)
D)Usain Bolt, who has a mass of approximately 94 kg, running at 10 m/s (22.4 miles per hour)
E)an oil tanker with a mass of 3 -10⁷ kg traveling at 9 m/s (20 miles per hour)

Question 56

If the speed of an object triples, its kinetic energy

A)increases by a factor of 3.
B)increases by a factor of 9.
C)decreases by a factor of 3.
D)decreases by a factor of 9.
E)is unaffected.

Question 57

Solid carbon dioxide CO₂ can undergo sublimation to form gaseous CO₂.Which of the following statements is true?

A)In the solid phase, CO₂ molecules easily slip past each other, and there are areas of randomly ordered molecules.
B)In the gas phase, CO₂ molecules are strongly attracted to each other.
C)The motion of the CO₂ molecules in the solid phase is much more restricted than in the gas phase.
D)CO₂ molecules in the solid phase are easily compressed to smaller volumes.
E)The CO₂ molecules decompose to form carbon and oxygen when they enter the gas phase.

Question 58

Soft solder is a blended alloy of tin 7.31 g/cm³) and lead 11.34 g/cm³) that is used in plumbing and electronics.It is 63.5% tin by mass.What is the density of the alloy?

A)9.87 g/cm³
B)8.27 g/cm³
C)7.83 g/cm³
D)8.79 g/cm³
E)9.33 g/cm³

Question 59

Which of the following is an example of potential energy?

A)water running down a hill
B)chemical bonds in table sugar sucrose
C)electrons flowing through a wire
D)a crowd moving a barricade
E)molecules moving randomly in a liquid

Question 60

At what velocity would a proton be traveling if it had the same kinetic energy as an electron traveling at 10.0% of the speed of light? KE = ½ mu², where m is the mass and u is the velocity; proton mass = 1.673 *10^-27 kg; electron mass = 9.109 * 10^-31 kg; speed of light = 2.998 -10⁸ m/s.

A)4.89 *10¹¹ m/s
B)2.45 * 10¹¹ m/s
C)4.95 * 10⁵ m/s
D)7.00 * 10⁵ m/s
E)3.50 *10⁵ m/s

Question 61

If the following arithmetic operations are carried out, how many significant figures should be reported in the answer?

A)1
B)2
C)3
D)4
E)5

Question 62

The average volume of a red blood cell is approximately 90 fL.Express the average value in liters using correct exponential notation and number of significiant figures.

A)90 *10^-15 L
B)9 *10^-15 L
C)9.0 * 10^-15 L
D)9 * 10^-14 L
E)9.0 * 10^-14 L

Question 63

The distance between the two hydrogen atoms in a water molecule is about 1.355 *10^-10 m.This is equal to _______.

A)1.355 *10^-8 mm.
B)1.355 *10⁶ cm.
C)1.355 * 10^-6 $\mu$ m.
D)13.55 nm.
E)135.5 pm.

Question 64

Green light in the visible portion of the electromagnetic radiation spectrum has wavelengths around 550 nm.Express this wavelength in meters using exponential notation.

A)5.5 * 10^-9 m
B)5.5 * 10^-7 m
C)5.5 m
D)5.5 * 10⁷ m
E)5.5 * 10⁹ m

Question 65

A student performed three measurements to determine the density of water at 25 $\degree$ C to four significant figures.The known density of water at 25 $\degree$ C to three significant figures is 0.997 g/mL.The student obtained the following results. The measurements were _______.

A)sufficiently precise but not accurate.
B)sufficiently accurate but not precise.
C)both sufficiently precise and accurate.
D)neither sufficiently precise nor accurate.
E)not repeated an adequate number of times.

Question 66

The average diameter of a red blood cell is about 7 *10^-6 m.Choose the best way to represent this distance using SI units and prefixes.

A)7 µm
B)0.007 mm
C)0.000007 m
D)7000 nm
E)7000000 pm

Question 67

If the following arithmetic operations are carried out, how many significant figures should be reported in the answer?
32 +0.56 + 0.210+ 3.3

A)1
B)2
C)3
D)4
E)5

Question 68

A graduated cylinder is filled with water to the 25.0 mL mark.After 27.5 g of titanium dioxide TiO₂ is added, the volume is 31.5 mL.Calculate the density of TiO₂.

A)0.873 g/cm³
B)0.87 g/cm³
C)4.2 g/cm³
D)4.23 g/cm³
E)2.05 g/cm³

Question 69

Which of the following is not an SI base unit?

A)( $\degree$ C)
B)s
C)kg
D)mol
E)m

Question 70

Which of the following common laboratory devices will deliver 25 mL of a solution with the greatest precision?

A)a 100 mL beaker without volume divisions
B)a 50 mL beaker with volume divisions every 10 mL
C)a 50 mL graduated cylinder with volume divisions every 2 mL
D)a 25 mL beaker without volume divisions
E)a 25 mL pipet with a to-deliver error of 0.01 mL

Question 71

Which of the following does not show a correct relationship between units?

A)1*10³ g = 1 kg
B)1 * 10^-3 s = 1 ms
C)1 nm = 1 * 10^-9 m
D)1 GB = 1 * 10⁹ B
E)1 * 10^-6 µL = 1 L

Question 72

Based on the following figure, which of the measurements listed is the best estimate of the length of the object?

A)1.8 cm
B)1.81 cm
C)1.810 cm
D)1.90 cm
E)1.9 cm

Question 73

What value should be reported for the total mass of three samples of iron weighing 117.0 g, 19.43 g, and 6.1043 g?

A)143 g
B)142.53 g
C)142.534 g
D)142.5 g
E)142.5343 g

Question 74

An 84.6419 g antique coin is thought to be gold.When the coin is placed in a graduated cylinder containing 15.53 mL of water, the water level rises to 24.64 mL.Calculate the density of the coin.

A)9.29 g/mL
B)5.450 g/mL
C)0.73833 g/mL
D)9.2911 g/mL
E)3.435 g/mL

Question 75

Which of the following represents the smallest mass?

A)4.0 *10⁰ mg
B)4.0 *10² ng
C)4.0 *10^-4 g
D)4.0* 10² F $\mu$ g
E)4.0*10^-6 kg

Question 76

The calculated diameter of a carbon atom is about 0.000000000340 m.In correct scientific notation, this is equal to _______.

A)3.40 * 10^-12 km.
B)3.40 * 10^-12 cm.
C)3.40 * 10^-8 mm.
D)3.40 * 10⁰ nm.
E)3.40 *10² pm.

Question 77

White fuming nitric acid should contain no more than 2% water by mass.The water content in four samples was measured.What is the average value, and which measured value is closest to the average?

A)1.953, sample 4
B)1.95, sample 4
C)1.9530, sample 4
D)1.9530, sample 3
E)1.953, sample 3

Question 78

A rectangular sheet of aluminum foil has a length of 8.0 cm, a width of 4.0 cm, and a mass of 864 mg.Determine the thickness of the foil, given that the density of aluminum is 2.70 g/cm³.

A)1.0 mm
B)0.10 mm
C)0.010 mm
D)10. $\mu$ m
E)1.0 *10² cm

Question 79

Which of the following does NOT show an exact relationship?

A)100 cm = 1 m
B)1 m³ = 1000 L
C)1 in = 2.54 cm
D)1 km = 0.6214 mi
E)1 dozen = 12 objects

Question 80

Which of the following represents the largest mass?

A)250 ng
B)25 µg
C)2.5 g
D)0.25 kg
E)25 mg